Q: The solubility product constant ($$K_{sp}) $$for $$BaSO_4 is$$ $$1.1 \times 10$$^{-10}$$. What is the molar solubility of $$BaSO_4$$ in pure water?

$$1.1 \times 10$$^{-5}$$~\mathrm{mol/L}$$

Q: A solution contains $$0.10~\mathrm{M}$$ $$NaF. $$What is the minimum concentration of $$Mg^{2+}$$ that must be added to initiate precipitation of $$MgF_2$$? ($$K_{sp} = 6.9 \times 10$$^{-9}$$)

$$6.9 \times 10$$^{-7}$$~\mathrm{M}$$

Q: Calculate the concentration of $$Cl^-$$ ions in a saturated solution of $$PbCl_2 if$$ $$K_{sp} = 2.4 \times 10$$^{-4}$$.

$$7.8 \times 10$$^{-2}$$~\mathrm{M}$$

Q: A solution contains $$0.050~\mathrm{M}$$ $$Mg^{2+}$$ ions. $$NaOH is $$added until the pH reaches $$11.0$$, causing $$Mg(OH)_2 to $$precipitate. What concentration of $$Mg^{2+}$$ will remain in solution at this pH? ($$K_{sp}(Mg(OH)_2) = 1.2 \times 10$$^{-11}$$)

$$1.2 \times 10$$^{-5}$$~\mathrm{M}$$

Q: Which of the following complex ions is the least stable in aqueous solution?

$$Cu(NH_3$)_4$$^{2+}$$, K_f = 5.0$$ \times $$10^{13}$$

Q: A solution contains $$0.10~\mathrm{M}$$ $$NaCl. $$What is the minimum concentration of $$Tl^+$$ ion required to initiate precipitation of $$TlCl$$? ($$K_{sp} = 1.8 \times 10$$^{-4}$$)

$$1.8 \times 10$$^{-3}$$~\mathrm{M}$$

Q: Given $$K_{sp}$$ for $$AgBr is$$ $$7.7 \times 10$$^{-13}$$ and K_f$ for Ag$$($$NH_3)_2$$^+$$ is 1.5$$ \times $$10^7$$, what is the molar solubility of $$AgBr in$$ $$5.0~\mathrm{M}$$ $$NH_3$$?

$$1.7 \times 10$$^{-2}$$~\mathrm{mol/L}$$

Question 1

A saturated solution of silver carbonate ($$Ag_2CO_3) is $$prepared. What is the correct relationship between the molar solubility $$s$$ and the concentration of $$Ag^+$$ ions in the solution?

Accepted Answer

$$0.5[Ag^+] = s$$

Question 2

The solubility product constant ($$K_{sp}) $$for $$BaSO_4 is$$ $$1.1 	imes 10$$^{-10}$$. What is the molar solubility of $$BaSO_4$$ in pure water?

Accepted Answer

$$1.1 	imes 10$$^{-5}$$~\mathrm{mol/L}$$

Question 3

Which of the following salts would be significantly more soluble in acidic solution than in pure water?

Accepted Answer

Only $$PbCO_3$$ and $$PbS$$

Question 4

A solution contains $$0.10~\mathrm{M}$$ $$NaF. $$What is the minimum concentration of $$Mg^{2+}$$ that must be added to initiate precipitation of $$MgF_2$$? ($$K_{sp} = 6.9 	imes 10$$^{-9}$$)

Accepted Answer

$$6.9 	imes 10$$^{-7}$$~\mathrm{M}$$

Question 5

Which of the following would decrease the $$K_{sp}$$ for $$PbI_2$$?

Accepted Answer

None of the above – the $$K_{sp} of a $$compound is constant at constant temperature.

Question 6

Calculate the concentration of $$Cl^-$$ ions in a saturated solution of $$PbCl_2 if$$ $$K_{sp} = 2.4 	imes 10$$^{-4}$$.

Accepted Answer

$$7.8 	imes 10$$^{-2}$$~\mathrm{M}$$

Question 7

A student mixes $$300~\mathrm{mL} of$$ $$1.1 	imes 10$$^{-3}$$~\mathrm{M}$$ $$MgCl_2$$ with $$500~\mathrm{mL} of$$ $$1.2 	imes 10$$^{-3}$$~\mathrm{M}$$ $$NaF. $$Will a precipitate of $$MgF_2$$ form? ($$K_{sp}($$MgF_2$$) = 6.9 	imes 10$$^{-9}$$)

Accepted Answer

No; $$Q \u003c K_{sp}$$

Question 8

Which one of the following solids would be more soluble in acidic solution than in neutral water?

Accepted Answer

$$CH_3COOK$$

Question 9

Given $$K_{sp}$$ for $$NiCO_3 is$$ $$6 	imes 10$$^{-9}$$ and K_f$ for Ni$$($$NH_3$$)_$$6^{2+} is$$ $$5 	imes 10^8$, what is the equilibrium constant K_c$ for the reaction: $$NiCO_3$$(s) + 6NH_3(aq) ightleftharpoons Ni(NH_3$)_6$$^{2+}$$(aq) + CO_3$^{2-}(aq)$$?

Accepted Answer

$$3.0$$

Question 10

A solution contains $$0.050~\mathrm{M}$$ $$Mg^{2+}$$ ions. $$NaOH is $$added until the pH reaches $$11.0$$, causing $$Mg(OH)_2 to $$precipitate. What concentration of $$Mg^{2+}$$ will remain in solution at this pH? ($$K_{sp}(Mg(OH)_2) = 1.2 	imes 10$$^{-11}$$)

Accepted Answer

$$1.2 	imes 10$$^{-5}$$~\mathrm{M}$$

Question 11

Which of the following best explains why $$CaCO_3 is $$more soluble in $$0.1~\mathrm{M}~HCl$$ than in pure water?

Accepted Answer

The $$H^+$$ ions react with $$CO_3$$^{2-}$$, shifting the dissolution equilibrium to the right.

Question 12

Which of the following complex ions is the least stable in aqueous solution?

Accepted Answer

$$Cu(NH_3$)_4$$^{2+}$$, K_f = 5.0$$ 	imes $$10^{13}$$

Question 13

A saturated solution of $$Ag_2SO_4 is $$prepared. What is the correct relationship between the molar solubility $$s$$ and the $$[Ag^+]$$ concentration?

Accepted Answer

$$[Ag^+] = 2s$$

Question 14

Which one of the following salts will be more soluble in acidic solutions than in basic solutions?

Accepted Answer

$$Ca_3$$($$PO_4)_2$

Question 15

A solution contains $$0.10~\mathrm{M}$$ $$NaCl. $$What is the minimum concentration of $$Tl^+$$ ion required to initiate precipitation of $$TlCl$$? ($$K_{sp} = 1.8 	imes 10$$^{-4}$$)

Accepted Answer

$$1.8 	imes 10$$^{-3}$$~\mathrm{M}$$

Question 16

Which of the following best describes the effect of adding $$NH_3 to a $$saturated solution of $$AgBr$$?

Accepted Answer

The solubility of $$AgBr$$ increases due to formation of $$[Ag(NH_3$)_2]^+$$ complex.

Question 17

Given $$K_{sp}$$ for $$AgBr is$$ $$7.7 	imes 10$$^{-13}$$ and K_f$ for Ag$$($$NH_3)_2$$^+$$ is 1.5$$ 	imes $$10^7$$, what is the molar solubility of $$AgBr in$$ $$5.0~\mathrm{M}$$ $$NH_3$$?

Accepted Answer

$$1.7 	imes 10$$^{-2}$$~\mathrm{mol/L}$$

Question 18

Which of the following best explains why $$BaSO_4 is $$least soluble in $$1.0~\mathrm{M}~H_2SO_4$$?

Accepted Answer

The high $$SO_4$$^{2-}$$ concentration shifts the equilibrium to favor the solid.

Question 19

A solution contains $$0.20~\mathrm{mol}$$ $$Co(NO_3$)_3 in$$ $$1.0~\mathrm{L} of$$ $$2.0~\mathrm{M}$$ $$NH_3$$. $$K_f$$ for $$Co(NH_3$)_6$$^{3+}$$ is 5.0$$ 	imes $$10^{31}. $$What is the concentration of free $$Co^{3+}$$ ions?

Accepted Answer

$$1.5 	imes 10$$^{-32}$$~\mathrm{M}$$

Question 20

Which of the following best describes the effect of the common ion on the solubility of $$MgF_2 in$$ $$0.10~\mathrm{M}$$ $$NaF$$?

Accepted Answer

The solubility decreases due to the common ion effect.

Solubility Equilibria and Solubility Product (Ksp) – Step-by-Step Study Guidance

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